This 3 sentence summary provides the key information from the document: The document consists of instructions for a chemistry exam, outlining that students should write their identification details on all work, use blue or black pen with pencil for diagrams, and answer all questions. It details the format of the exam, including the use of calculators and showing working, and instructs students to fasten their work together at the end. The exam consists of 6 questions investigating various chemistry concepts and reactions through experiments and analysis.

1. READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use a pencil for any diagrams, graphs or rough working.
Do not use staples, paper clips, highlighters, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
Electronic calculators may be used.
You may lose marks if you do not show your working or if you do not use appropriate units.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
CHEMISTRY 0620/62
Paper 6 Alternative to Practical May/June 2013
1 hour
Candidates answer on the Question Paper.
No Additional Materials are required.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS
International General Certificate of Secondary Education
This document consists of 11 printed pages and 1 blank page.
[Turn over
IB13 06_0620_62/RP
© UCLES 2013
*2436679162*

2. 2
0620/62/M/J/13© UCLES 2013
For
Examiner’s
Use
1 A student extracted the colours present in some leaves using the apparatus below.
(a) Complete the boxes to identify the pieces of apparatus used. [2]
(b) Use labelled arrows to indicate
(i) the solvent,
(ii) the solution of colours. [2]
(c) Chromatography was used to separate the colours. The chromatogram obtained is
shown.
(i) On the diagram, label the solvent front. [1]
(ii) How many colours were present?
.............................................................................................................................. [1]
[Total: 6]

3. 3
0620/62/M/J/13© UCLES 2013 [Turn over
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Examiner’s
Use
2 A student investigated the reaction of methane, CH4, and copper(II) oxide. She passed
methane gas over hot copper(II) oxide using the apparatus shown.
excess methane
burning
methane
heat
copper(II) oxide
The solid changed colour to red-brown and drops of liquid condensed in the cold part of the
tube.
(a) What was the original colour of the solid?
..................................................................................................................................... [1]
(b) Suggest the identity of
(i) the red-brown solid, ...................................................................................................
(ii) the drops of liquid. ............................................................................................... [2]
(c) Suggest a physical test to identify the liquid.
test ....................................................................................................................................
result ........................................................................................................................... [2]
[Total: 5]

4. 4
0620/62/M/J/13© UCLES 2013
For
Examiner’s
Use
3 A student investigated the reaction between a solution of deep purple aqueous potassium
manganate(VII), and two different colourless solutions, B and C, of an acidic solution of a
sodium salt.
Two experiments were carried out.
Experiment 1
A burette was filled with the solution of potassium manganate(VII) to the 0.0cm3
mark.
Using a measuring cylinder, 25cm3
of solution B was poured into the conical flask.
The potassium manganate(VII) solution was added slowly to the flask and shaken to mix
thoroughly. Addition of the solution was continued until there was a permanent pink colour in
the contents of the flask.
(a) Use the burette diagram to record the volume in the table of results and complete the
table.
25
26
27
final reading
final reading/cm3
initial reading/cm3
difference/cm3
[2]
Experiment 2
Experiment 1 was repeated using solution C instead of solution B.
(b) Use the burette diagrams to record the volumes in the table and complete the table.
31
32
33
initial reading
18
19
20
final reading
final reading/cm3
initial reading/cm3
difference/cm3
[2]

5. 5
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Examiner’s
Use
(c) (i) What colour change was observed in the contents of the flask when potassium
manganate(VII) solution was added to the flask in Experiment 1?
from ....................................................... to ........................................................ [1]
(ii) Why was an indicator not added to the flask?
.............................................................................................................................. [1]
(d) (i) In which experiment was the greater volume of potassium manganate(VII) solution
used?
.............................................................................................................................. [1]
(ii) Compare the volumes of potassium manganate(VII) solution used in Experiments 1
and 2.
.............................................................................................................................. [1]
(iii) Suggest an explanation for the difference in volumes in (d)(ii).
....................................................................................................................................
....................................................................................................................................
.............................................................................................................................. [2]
(e) If Experiment 2 was repeated using 12.5cm3
of solution C, what volume of potassium
manganate(VII) solution would be used? Explain your answer.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [3]
(f) A redox reaction occurs when potassium manganate(VII) reacts with solutions B and C.
Explain the term redox reaction.
...........................................................................................................................................
..................................................................................................................................... [2]
(g) Give one advantage and one disadvantage of using a measuring cylinder for solution C.
advantage .........................................................................................................................
disadvantage .............................................................................................................. [2]
[Total: 17]

6. 6
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Examiner’s
Use
4 A mixture of two solids, R and S, was analysed.
Solid R was the water-soluble salt aluminium sulfate, Al2(SO4)3, and solid S was an insoluble
salt.
The tests on the mixture and some of the observations are in the following table.
Complete the observations in the table.
tests observations
Distilled water was added to the mixture in a
boiling tube.
The boiling tube was shaken and the contents
of the boiling tube filtered, keeping the filtrate
and residue for the following tests. The filtrate
was divided into five test-tubes.
tests on the filtrate
(a) Appearance of the first portion of the
filtrate. ............................................................ [1]
(b) Drops of aqueous sodium hydroxide were
added to the second portion of the solution
and the test-tube shaken.
Excess aqueous sodium hydroxide was
then added to the test-tube.
...................................................................
............................................................ [3]
(c) Aqueous ammonia was added to the third
portion, dropwise and then in excess.
...................................................................
............................................................ [2]
(d) Dilute nitric acid was added to the fourth
portion of the solution followed by aqueous
silver nitrate. ............................................................ [1]
(e) Dilute nitric acid was added to the fifth
portion of the solution and then aqueous
barium nitrate. ............................................................ [2]

7. 7
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Examiner’s
Use
tests observations
tests on the residue
(f) Dilute hydrochloric acid was added to the
residue.
The gas given off was tested.
Excess aqueous sodium hydroxide was
added to the mixture in the test-tube.
rapid effervescence
limewater turned milky
white precipitate, insoluble in excess
(g) Name the gas given off in test (f).
..................................................................................................................................... [1]
(h) What conclusions can you draw about solid S?
..................................................................................................................................... [2]
[Total: 12]

8. 8
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For
Examiner’s
Use
5 A student investigated the temperature changes when dilute nitric acid neutralised aqueous
potassium hydroxide. The instructions followed are listed below.
Step 1 The solutions were left at room temperature for one hour.
Step 2 Using a measuring cylinder, 20cm3
of aqueous potassium hydroxide solution was
poured into a polystyrene cup and its temperature measured.
Step 3 From a burette, 5.0cm3
of nitric acid was added to the cup. The highest temperature
reached by the mixture was measured. A further 5.0cm3
of nitric acid was added to
the mixture and the highest temperature measured. Further 5.0cm3
additions were
made until a total of 30.0cm3
of nitric acid had been added.
(a) Use the thermometer diagrams to complete the temperatures in the table.
volume of nitric acid
added/cm3
thermometer
diagram
highest temperature
reached/°C
0.0
30
25
5.0
30
25
10.0
40
35
15.0
45
40
20.0
45
40
25.0
40
35
30.0
40
35
[3]

9. 9
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Examiner’s
Use
(b) Plot the results on the grid. Draw two intersecting straight lines through the points.
0 5 10 15 20 25 30
50
40
30
20
10
highest
temperature
reached/°C
total volume of nitric acid/cm3
[4]
(c) From your graph, work out the volume of nitric acid needed to completely neutralise the
20cm3
of aqueous potassium hydroxide. Using an arrow, show clearly on the grid this
neutralisation point.
..................................................................................................................................... [2]
(d) What was the room temperature?
..................................................................................................................................... [1]
(e) Why was a polystyrene cup used instead of a glass beaker?
..................................................................................................................................... [1]

10. 10
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(f) Why does the temperature:
increase ............................................................................................................................
...........................................................................................................................................
then decrease? .................................................................................................................
..................................................................................................................................... [2]
(g) What type of chemical reaction is this neutralisation?
..................................................................................................................................... [1]
[Total: 14]

11. 11
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For
Examiner’s
Use
6 Two metals, A and B, each react with dilute sulfuric acid to produce hydrogen.
Plan an investigation to show which metal, A or B, is the more reactive metal. You may
include a diagram in your answer.
You are provided with:
● standard laboratory equipment
● powdered metals A and B
● dilute sulfuric acid.
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
..................................................................................................................................................
............................................................................................................................................ [6]
[Total: 6]

12. 12
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reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the
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University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of
Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
0620/62/M/J/13
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